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Ch.17 - Applications of Aqueous Equilibria
McMurry - Chemistry 8th Edition
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Tutti i libri di testoMcMurry 8th EditionCh.17 - Applications of Aqueous EquilibriaProblema 12
Capitolo 17, Problema 12

What is the solubility-constant expression for Ca3(PO4)2 (s)? (a) [Ca2+]3 [PO43-]2 (b) [Ca2+]3 [PO43-]2 / [Ca3(PO4)2] (c) [Ca(PO4)2] / [Ca2+]3 [PO43-]2 (d) [Ca2+]2 [PO43-]3

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1
Identify the chemical formula of the compound: \( \text{Ca}_3(\text{PO}_4)_2 \).
Recognize that the solubility product constant \( K_{sp} \) is used for sparingly soluble salts and involves the concentrations of the ions in solution.
Write the dissociation equation for \( \text{Ca}_3(\text{PO}_4)_2 \): \( \text{Ca}_3(\text{PO}_4)_2 (s) \rightleftharpoons 3\text{Ca}^{2+} (aq) + 2\text{PO}_4^{3-} (aq) \).
Express the solubility product constant \( K_{sp} \) as the product of the concentrations of the ions, each raised to the power of their coefficients in the balanced equation: \( K_{sp} = [\text{Ca}^{2+}]^3 [\text{PO}_4^{3-}]^2 \).
Compare the expression with the given options to identify the correct one.

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Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that applies to the solubility of sparingly soluble ionic compounds. It is defined as the product of the molar concentrations of the ions, each raised to the power of their coefficients in the balanced dissolution equation. For a compound like Ca3(PO4)2, Ksp helps predict how much of the solid can dissolve in water.
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Solubility Product Constant

Dissociation of Ionic Compounds

When ionic compounds dissolve in water, they dissociate into their constituent ions. For calcium phosphate, Ca3(PO4)2, the dissociation can be represented as Ca3(PO4)2 (s) ⇌ 3 Ca2+ (aq) + 2 PO4^3- (aq). Understanding this dissociation is crucial for writing the correct Ksp expression, as it directly relates to the concentrations of the ions in solution.
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Ionic Compounds Naming

Equilibrium Expressions

Equilibrium expressions are mathematical representations of the concentrations of reactants and products at equilibrium. For Ksp, the expression is formed by taking the concentrations of the ions produced from the dissolution of the solid, raised to their respective stoichiometric coefficients. This concept is essential for determining the correct form of the Ksp expression for any given ionic compound.
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Equilibrium Constant Expressions
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The pH titration curve applies to the titration of 40.0 mL of a 0.100 M solution of an acid with 0.100 M NaOH. What are the approximate pKa values for this acid?

(a) pKa1 = 5, pKa2 = 10 (b) pKa1 = 7, pKa2 = 11 (c) pKa1 = 5, pKa2 = 10, pKa3 = 13 (d) pKa1 = 5, pKa2 = 7, pKa3 = 10
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